NH3 is a weak base (Kb=1.8×10−5 M), so the salt NH4Cl acts as a weak acid. What is the pH of a solution that is 0.075 Min NH4Cl?

Q: The base constant for ammonia, NH3, is Kb = 1.8 x 10-5. A solution was made up with ammonium…

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Q: The Ka, for propionic acid, HC3H5O2, is 1.30 x 10^ -5. What is the pH of a 0.0850 M propionic acid…

A: The dissociation reaction of propanoic acid is given by  HC3H5O2 -----> H+ + C3H5O2- hence Ka = […

Q: what is the pH of a solution obtained by mixing 225 mL of 0.680 M HCl with 565 mL of an HCl solution…

A: Here, we have to calculate the pH of a solution obtained by mixing 225 mL of 0.680 M HCl with 565 mL…

Q: NH3 is a weak base (?b=1.8×10^−5) and so the salt NH4Cl acts as a weak acid. What is the pH of a…

A: Given: Kb = 1.8 × 10-5              Concentration of solution = 0.056 M             Temperature = 25…

Q: A 0.107 M solution of Providenol, a weak acid, has a measured pH of 4.32. Determine the pKa of…

A: The equilibrium constant depicting dissolution of either weak acids/base is known as dissociation…

Q: What is the pH of a solution in which 15 mL of 0.39 M NaOH is added to 25 mL of 0.39 M HCl?

A: Since NaOH and HCl are strong base and acid respectively Hence they will react as per the reaction…

Q: Explain why the pH does not change significantly when a small amount of an acid or a base is added…

A: The solution of a weak acid or base with its conjugate base or acid respectively is known as a…

Q: What is the pH of a solution that contains 0.10 M cyanic acid and 0.20 M sodium cyanate?

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Q: HCN is a weak acid (Ka=6.20×10−10), so the salt, KCN , acts as a weak base. What is the pH of a…

A: Ka = 6.20×10-10 pKa = -log(Ka)    = -log(6.2×10-10 = 9.21  Concentration(C) of salt =0.0750 M

Q: What is the pH in a solution consisting of Ba(OH)2 6.17x10-8M.

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Q: Barbituric acid, HC4H3N2O3, is a weak acid that is used to prepare various barbiturate drugs (used…

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Q: Sid What is the pH of ammonium bromide solution with a concentration of 0.563 M. The base ionization…

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Q: The pH of a white vinegar solution is 2.20. This vinegar is an aqueous solution of acetic acid with…

A: Concentration of H+ can be calculated as follows:

Q: The pH of a solution of household ammonia, a 0.950-M solution of NH3, is 11.612. What is Kb for NH3.

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Q: HCl is a strong acid.  What is the pH of a solution of concentration 1 x 10-3M?

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Q: Identify the major species present in each solution. The strongest acid will react with the…

A: 0.12 M KNO2 b. 0.45 M NaOCl c. 0.40 M NH4ClO4

Q: What is the pH of 500 mL of water after the addition of 50 mL of 25 mM HCl?

A: Since,      Numbers of moles  =  Molarity solution×volume of solution                   of…

Q: Calculate the pH of each of the following solutions of a strong acid in water. (a) 0.22 М HCI (b)…

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Q: NH3 is a weak base (?b=1.8×10^5) and so the salt NH4Cl acts as a weak acid. What is the pH of a…

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Q: HClO is a weak acid (?a=4.0×10^−8) and so the salt NaClO acts as a weak base. What is the pH of a…

A: Given : Concentration of NaClO = 0.014 M Since NaClO is a weak conjugate base of weak acid HClO.…

Q: Novocaine, C13H21O2N2Cl, is the salt of the base procaine and hydrochloric acid.  The Kb of procaine…

A: Salts are of three types .They are Acidic salt , basic salt and neutral salt.

Q: List the acidic salts in increasing order of acid strength, then list the basic salts in increasing…

A: Acid are the substance which donates proton in the aqueous solution. Example:HCl(aq)→H+(aq)+Cl-(aq)…

Q: What is the pH of a 0.30 M solution of methylammonium chloride, CH3NH3CL?  What is the…

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Q: A 2.5-g quantity of HCl is dissolved in 245 mL of water and then diluted to 890 mL. What is the pH…

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Q: Identify the following as acidic or basic, and write the corresponding Ka or Kb reactions and…

A: (a) HF is a weak acid.  the reaction is : HF (aq) + H2O (l) ---------> H3O+ (aq) + F– (aq) Ka…

Q: Explain why the pH does not change significantly when a small amount of an acid or a base is added…

A: A mixture of weak acid and its salt forms a buffer solutions or buffers.  Buffers solutions resist…

Q: A solution of acetic acid (Ka = 1.8 × 10‒5) has a pH of 2.65. What is the concentration of acetic…

A: Given information: Ka of acetic acid = 1.8 × 10‒5 pH is 2.65

Q: What is the pH of a solution made by mixing 23.9g of ammonium nitrate with enough water to make…

A: In this questions the hydrolysis of salt take place .The NH4+ will be hydrolyzed with water. So be…

Q: Which are Lewis acids and which are Lewis bases?(a) Mg²⁺(b) OH⁻(c) SiF₄(d) BeCl₂

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Q: Calculate the pH of a 0.50 M solution of sodium cyanide (NaCN). The K, of HCN is 4.9 x 10 10.

A: A strong base and weak acid react to form salt and water. The salt will be basic in nature and the…

Q: NH3 is a weak base (Kb=1.8×10−5Kb=1.8×10−5) and so the salt NH4Cl acts as a weak acid. What is the…

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Q: What is the pH of a solution obtained by adding 222 mL of 0.111 M  HCl to 596 mL of a HNO3 solution…

A: Since both HNO3 and HCl are strong acids Hence they will dissociate completely in solution  Hence…

Q: At 25 °C, how many dissociated OH– ions are there in 1291 mL of an aqueous solution whose pH is…

A: The number of dissociated hydroxide ions are present in given solution is determined as,

Q: 500

A: Dear student I have given answer to your question in the image format.

Q: HCN is a weak acid (Ka=6.20×10−10) , so the salt, KCN , acts as a weak base. What is the pH of a…

A: Weak acid are those acid which does not dissociate completely in aqueous solution and weak base are…

Q: What is the pH of a solution that is 0.34 M KOCN and 0.14 M HOCN (cyanic acid)?

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Q: A solution is prepared by adding 500 mL of 0.30 M NaCN(aq) to 500 mL of 0.40 M HCN(aq) at 25 degrees…

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Q: HCNN is a weak acid (?a=6.20×10^−10) , so the salt, KCN , acts as a weak base. What is the pH of a…

A: Given: Ka of HCN = 6.20×10-10 KCN = 0.0525 M we have to determine the pH ? Kb = Kw / Ka       = 1 ×…

Q: When 0.100 moles of NaX salt are dissolved in water to a volume of 1.00L, the pH and solution is…

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Q: What is the pH of an aqueous solution at 25 °C that contains 2.5x10-4 hydronium ion

A: pH is used to measure the concentration of hydronium ion. The expression for calculating the pH of…

Q: What is the pH of a solution made by mixing 45.00mL of 0.1256M HCl with 20.00mL of 0.2006M NH3?

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Q: Sodium hydroxide is a strong base. What is pH of a 0.02M sodium hydroxide solution?

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Q: NH3 is a weak base (?b=1.8×10−5Kb=1.8×10−5) and so the salt NH4Cl acts as a weak acid. What is the…

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Q: Calculate the equilibrium concentration of the nonionized bases and all ions in a solution that is…

A: Given that: concentration of NH3 = 0.115 M concentration of C6H5NH2 =  0.100 M To find:…

Q: What is the pH of a solution that is 0.041 M in NH4Cl?

A: NH4Cl salt can be formed from weak base NH4OH and strong acid HCl. So it is a salt of strong acid…

Q: What is the pH of ammonium bromide solution with a concentration of 0.563 M. The base ionization…

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Q: What is the concentration of hydroxide ion in a 0.150 M aqueous solution of hydroxylamine, NH,OH?…

A: NH4OH is a weak base, hence it can't dissociate completely, hence equilibrium is established between…

Q: HCIO is a weak acid (K, = 4.0 x 10-) and so the salt NaCIO acts as a weak base. What is the pH of a…

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Q: NH3 is a weak base (Kb = 1.8 × 10–5) and so the salt NH4Cl acts as a weak acid. What is the pH of a…

A: Dissociation constant of base is given by,

Q: 1. Which has the lowest pH? Explain why. 0.10M HCl or 0.20M HCl

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Ionic Equilibrium

Chemical equilibrium and ionic equilibrium are two major concepts in chemistry. Ionic equilibrium deals with the equilibrium involved in an ionization process while chemical equilibrium deals with the equilibrium during a chemical change. Ionic equilibrium is established between the ions and unionized species in a system. Understanding the concept of ionic equilibrium is very important to answer the questions related to certain chemical reactions in chemistry.

Arrhenius Acid

Arrhenius acid act as a good electrolyte as it dissociates to its respective ions in the aqueous solutions. Keeping it similar to the general acid properties, Arrhenius acid also neutralizes bases and turns litmus paper into red. 

Bronsted Lowry Base In Inorganic Chemistry

Bronsted-Lowry base in inorganic chemistry is any chemical substance that can accept a proton from the other chemical substance it is reacting with.